A container of volume $200 ext{ cm}^3$ contains 0.2 mole of hydrogen gas and 0.3 mole of argon gas. The pres

Question

A container of volume $200 	ext{ cm}^3$ contains 0.2 mole of hydrogen gas and 0.3 mole of argon gas. The pressure of the system at temperature $200 	ext{ K}$ ($R = 8.3 	ext{ J K}^{-1} 	ext{ mol}^{-1}$) will be:

Accepted Answer

According to Dalton's Law of Partial Pressures, the total pressure exerted by a mixture of non-reactive gases is the sum of the partial pressures of individual gases. Alternatively, using the Ideal Gas Equation $PV = nRT$ for the total mixture:

1.  **Calculate Total Moles ($n$):**
    $n = n_{H_2} + n_{Ar} = 0.2 + 0.3 = 0.5 	ext{ mol}$

2.  **Convert Volume to SI Units ($V$):**
    $V = 200 	ext{ cm}^3 = 200 	imes 10^{-6} 	ext{ m}^3 = 2 	imes 10^{-4} 	ext{ m}^3$

3.  **Apply Ideal Gas Equation:**
    $P = \frac{nRT}{V}$
    $P = \frac{0.5 	imes 8.3 	imes 200}{2 	imes 10^{-4}}$
    $P = \frac{830}{2 	imes 10^{-4}}$
    $P = 415 	imes 10^4 	ext{ Pa}$
    $P = 4.15 	imes 10^6 	ext{ Pa}$

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